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Barium chloride (BaCl₂) is one of the most prevalent barium salts that's water soluble. It's white, highly toxic, and gives a flame a yellow-green tint like most other water-soluble barium salts. It's also hygroscopic, forming the dihydrate BaCl₂(H₂O)₂ first. Orthorhombic cotunnite (PbCl₂) and cubic fluorite (CaF₂) are the two polymorphs (or forms) that it crystallises in. It can be utilised in a variety of sectors, including testing sulphate ions in laboratories and purifying brine solution in the pigment manufacturing process, as well as other barium salts. It's poisonous, cheap, and produces a yellow-green flame.
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Key Terms: Barium dichloride, Barium Chloride, Structure, Preparation, Uses, Properties, Toxicity, pH.
Barium Chloride
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The inorganic compound barium chloride has the formula BaCl₂. It's one of the most prevalent barium salts that's water soluble. It's poisonous, like other barium salts, and gives a flame a yellow-green hue. It also has a high hygroscopicity. Wastewater treatment, the manufacturing of PVC stabilisers, oil lubricants, barium chromate, and barium fluoride are all applications for barium chloride dihydrate.
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Structure of Barium Chloride
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BaCl₂ crystallises in two different shapes (polymorphs). The cubic fluorite (CaF₂) structure is found in one form, whereas the orthorhombic cotunnite (PbCl₂) structure is found in the other. Both polymorphs account for the big Ba²⁺ ions predilection for coordination numbers greater than six. In the fluorite structure, Ba²⁺ has a coordination of 8 while in the cotunnite structure, it has a coordination of 9. When cotunnite-structure BaCl₂ is subjected to pressures of 7–10 GPa, it converts into a monoclinic post-cotunnite phase, which is a third structure. The number of Ba²⁺ coordination increases from 9 to 10.
Structure of Barium Chloride
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Properties of Barium Chloride
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Following are the properties of Barium Chloride:
- BaCl₂ behaves as a simple salt in aqueous solution; it is a 1:2 electrolyte in water and has a neutral pH. Its solutions react with the sulphate ion to form a thick white barium sulphate precipitate.
| Ba2+ + SO2−4 → BaSO4 |
- Oxalate effects a similar reaction:
| Ba2+ + C2O2−4 → BaC2O4 |
- When combined with sodium hydroxide, it produces hydroxide, which is water soluble to a degree.
- Melting Point and Boiling Point of Barium Chloride are 962 degree Celsius and 1560 degree Celsius respectively.
- Density of Anhydrous Barium Chloride is 3.856 g/cm3.
- Molecular Weight of Anhydrous Barium Chloride is 205.23 g/mol.
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Preparation of Barium Chloride
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It is made from barite (barium sulphate) in a two-step method on an industrial scale:
| BaSO4 + 4C → BaS + 4CO |
The first step requires a high temperature.
| BaS + 2HCl → BaCl2 + H2S |
Chlorine can be used instead of HCl.
It is possible to make barium chloride from barium hydroxide or barium carbonate. The reaction of these basic salts with hydrochloric acid generates hydrated barium chloride.
Uses of Barium Chloride
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Although inexpensive, barium chloride finds limited applications in the laboratory and industry:
- Barium chloride is primarily utilised in industry for the purification of brine solution in caustic chlorine facilities, as well as the creation of heat treatment salts and steel case hardening.
- Red pigments like Lithol red and Red Lake C are made from barium chloride (BaCl₂). Its usefulness is limited due to its toxicity.
The toxicity of this chemical restricts its use.
Toxicity of Barium Chloride
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When consumed, this chemical is poisonous. Magnesium sulphate (MgSO₄) and sodium sulphate (Na₂SO₄), which combine to generate BaSO₄, are likely antidotes (barium sulfate). Because of its insolubility, BaSO₄ is relatively non-toxic. BaCl₂, like most other barium salts, is extremely hazardous to humans. This chemical can irritate the eyes, mucous membranes, and skin when exposed to it. Barium chloride can also be lethal if consumed or inhaled. The central nervous system, the cardiovascular system, and the kidneys can all be harmed by barium chloride.
Things To Remember
- The inorganic compound barium chloride has the formula BaCl₂.
- Barium Chloride is poisonous, like other barium salts, and gives a flame a yellow-green hue.
- When consumed, this chemical is poisonous. Magnesium sulphate (MgSO₄) and sodium sulphate (Na₂SO₄), which combine to generate BaSO₄, are likely antidotes (barium sulphate).
- Although inexpensive, barium chloride finds limited applications in the laboratory and industry. The toxicity of this chemical restricts its use.
Sample Questions
Ques: What are the Uses of Barium Chloride? (2 Marks)
Ans: Despite its low cost, barium chloride is only used in a few industries and laboratories. It is largely used in industry for the purification of brine solution in caustic chlorine facilities, as well as for steel hardening and the manufacturing of heat treatment salts. The toxicity of this chemical restricts its use.
Ques: What is the pH of Barium Chloride? (2 Marks)
Ans: Ba2+ (aqueous) ions and Cl- ions are produced when barium chloride (BaCl₂) dissolves in water and ionises. Cl- and Ba2+ do not hydrolyze because they are the anion and cation of a strong acid and a strong base, respectively (or react with water). As a result, no more OH- or H+ is created, and the solution is neutral (with a pH of 7).
Ques: Why should Barium Chloride be Acidified? (2 Marks)
Ans: If it's going to be used for a sulphate test, it needs to be acidified because both sulphates and sulphites generate a white precipitate when tested with BaCi. Because the ppt dissolves in acids in the case of sulfites, acid is given to the Baci before testing to avoid misunderstanding in the findings.
Ques: How is Barium Chloride formed? (2 Marks)
Ans. The chemical formula for barium chloride is BaCl₂, and its molar mass is 208.23 g mol⁻¹. One barium cation (Ba2+) and one chlorine anion combine to make this salt (Cl-). The dihydrate form of barium salt has a molar mass of 244.26 g mol⁻¹.
Ques: What are the oxidation numbers of Ba and Cl in BaCl₂? (2 Marks)
Ans. The barium cations and chloride anions form an ionic connection in barium chloride molecules. In this ionic salt, barium is a metal with an oxidation state of +2, whereas chlorine is a non-metal with an oxidation state of -1 in BaCl₂.
Ques: Why is barium chloride toxic? (2 Marks)
Ans. Humans are badly poisoned by BaCl₂, as are most other barium salts. When exposed to this substance, it can irritate the eyes, mucous membranes, and skin. If ingested or inhaled, barium chloride can be fatal. Barium chloride can affect the central nervous system, the cardiovascular system, and the kidneys.
Ques: Stae the properties of aqueous solution of BaCl₂? (2 Marks)
Ans. Because they contain the cation of a strong base and the anion of a strong acid, aqueous solutions of barium chloride have a neutral pH. When barium sulphate is subjected to sulphates, it forms a white precipitate.
Ques: What is the procedure of producing Barium chloride industrially? (2 Marks)
Ans. A two-step procedure is used in the industrial manufacturing of barium chloride. At high temperatures, barium sulphate (typically in the form of the mineral barite) reacts with carbon to produce barium sulphide and carbon monoxide. The barium sulphide is then treated with hydrochloric acid to produce barium chloride and hydrogen sulphide.
Ques: What are the uses of Barium? (2 Marks)
Ans: (i) Barium is used in metallurgy, pyrotechnics, petroleum mining, and radiology.
(ii) It is also used as deoxidizers in copper refining.
(iii) When barium alloy is mixed with nickel, it emits an electron, which is used in electron tubes and sparks plug electrodes.
(iv) It acts as a scavenger with oxygen and other gases.
(v) An isotope of barium is used as a source of gamma rays.
Ques: List five compounds of barium with their chemical formula. (3 Marks)
Ans: (i) Barium chloride → BaCl₂
(ii) Barium chromate → BaCrO₄
(iii) Barium oxide → BaO
(iv) Barium hydroxide → Ba(OH)₂
(v) Barium sulphate → BaSO₄
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